For a fixed mass of gas at a constant temperature, what happens torb8d a chdi:7q9scz :. the volume if the pre:sichd ab9cd.rz8 7q:ssure of the gas is doubled?

  Which of the following conditionsuc-j5q(x w(mjsp(e*c 5s o;xi makes gases deviate from ideal behavior?

  Based on the graph below, choose the co40yq m gplh07calvchu20 mp 03rrect statement that describes the relationship be0g0mpc4luh7 pyv0aml0 c 2h3 qtween pressure and temperature for a fixed mass and volume of a gas?

  The ideal gas equation is a formula that combines t jrlzrp *61huk 37uo-she relationship between pressure, volume, tempjk3 z6hsuu l *rp1or-7erature, and the number of moles.
1.Complete the table below by calculating the missing variables of the ideal gas equation.

P	V	n	T
$\times10^4$Pa	$0.015m^3$	0.400mol	$37^{\circ}C$
152,000Pa	$m^3$	2.00mol	298.15K
31,000Pa	$0.25m^3$	mol	271.15K
250kPa	$0.75dm^3$	0.580m0l	k

2.A $256cm^3$ flask contains 0.800g of a gaseous compound with an empirical formula of CHCl. The pressure and the temperature of the gas are respectively $10^5$, Pa10 and 373K. Determine the molecular formula of the compound.

  Liquid butanol $(C_4H_9OH)$ burns or combusts in oxygen to produce $CO_{2(g)}$ and $H_2O$(g).
1.Write a balanced equation, including state symbols, for this reaction.
2.When $1.250cm^3$ of butanol is combusted in excess oxygen,$1.921dm^3$ of water vapor is collected at a pressure of 125.0 kPa and $150.0^{\circ}C$. Calculate the moles of butanol that were combusted.  mol
3.Determine the density of liquid butanol in $g\:cm^{-3}$.  g $cm^{-3}$

  Based on the table below, what is the corre yp1zt7rwfqq)ur8 2p1 ct calculation to determine the final volume of a fixed mass of gas: )8q puqr1y 2p7f1wr zt

Initial	Final
Pressure = 1.00 atm	Pressure = 1.60 atm
Temperature =$20^{\circ}C$	Temperature =$10^{\circ}C$
Volume =$5.00dm^3$	Volume = ?

  Automobile airbags are inflated wqf zh9rbc au 0,t)9kf-ith $N_2$, a byproduct of sodium azide decomposition, according to the following reaction.
$2NaN_{3(s)}\rightarrow2 Na_{(s)}+3N^{2(g)}$
Calculate the mass (in grams) of sodium azide needed to generate $0.07m^3$ of $N^2$ at $1.01\times10^{5}Pa$ and $26.0^{\circ}C$.$n_{N2}$=  mol, mass of $NaN_3$=  g

  14.01g of nitrogen gr-h vjoi 28 xjyms9c1 :zf hk:7)p6mua6ts m4gas $(N_2)$ is reacted with excess $H_2$. What volume of ammonia $(NH_3)$gas would be produced at STP? The molar volume of a gas at STP is $22.7dm^3$.
$N_{2(g)}+3H_{2(g)}\rightarrow2NH_{3(g)}$

  Sodium azide is an ionic compound found within the a8 2e d)w-pur/- c4ahc+oidbqd9 s iq7uirbags of some older cars. The airbag is deployed as a safety feature in the event of an acsi- 4p -u9qwr)duc7e2d/o 8 c+qbadhicident. In this application, the sodium azide decomposes rapidly, and the gas formed inflates the airbag.
The decomposition of sodium azide under these conditions is given below.
$2NaN_{3(s)}\rightarrow2Na (s)+3 N_{2(g)}$
1.Suggest the formula and charge for the azide ion.
2.A typical airbag requires $65.0dm^3$of nitrogen gas for complete inflation at STP. Using section 2 of the data booklet, calculate the mass of sodium azide that the airbag must contain for this purpose.Molar mass for sodium azide calculated=  $g mol^{-1}$

  Which of the following gases pxn7 crar+f l bln783j2c)y p,:ym*o5vp6qehmost closely aligns with the behavior of an ideal gas+,2nn76lxrby7f 8p r:h pco jevy*l3 qc5m) ap?

  Under which conditions would a gas devi;: cs4go19bdtbw t m.c:w)jawate the most from the ideal gas model?

  A sample of gas at a certain temperature, pressure, and voqpaiyjv h1//v2k-qw(-y6fquxhp ( , ylume $(T_1,P_1,and V_1T)$ undergoes a change in temperature and pressure $(T_2andP_2)$.What is the new volume $(V_2)$?
Before: $T_1,P_1,V_1$;
After: $P_2=2P_1$ AND $T_2=\frac{1}{2}T_1$